#### Universal gas constant : R_{u} = 8.314 kJ/(kmol K)

#### Absolute temperature : deg K = deg C + 273.15 K

but : 1 deg K temperature difference equals 1 deg C temperature
difference

#### Equations for ideal gases with constant specific heats

c_{p} = specific heat at constant pressure [kJ/(kg K)] , the amount
of heat you need to raise the temperature of 1 kg of gas by 1 deg K
while keeping the pressure constant despite the temperature change.

c_{v} = specific heat at constant volume [kJ/(kg K)] , the amount
of heat you need to raise the temperature of 1 kg of gas by 1 deg K
while keeping the volume constant despite the temperature change.

κ = c_{p} / c_{v} = ratio of above specific
heats.

&kappa = 1.6667 for mono-atomic ideal gases (He , Ne , Ar , Xe ...)

&kappa = 1.4000 for di-atomic ideal gases O_{2},
N_{2}, H_{2}, ....

Specific gas constant has different value for different gases :

R_{s} = R_{u} / M [kJ/( kg K )]

M = molecular mass (weight) [ kg/Kmol ]

Ideal gas law :

p*V = m*R_{s}*T

p*V = n*R_{u}*T

p = pressure [N/m^{2}]

V = volume [m^{3}]

m = mass [kg]

T = absolute temperature [K]

n = number of moles [kmol]

Zig Herzog; hgnherzog@yahoo.com
Last revised: 01/29/10